![SOLVED: Results: Calculate the heat gained by the water (lost by the substance in the calorimeter using the equation in the Introduction: Remember t0 write the unitsl! Q fon water using Ist SOLVED: Results: Calculate the heat gained by the water (lost by the substance in the calorimeter using the equation in the Introduction: Remember t0 write the unitsl! Q fon water using Ist](https://cdn.numerade.com/ask_images/ee5df36874cb4055adf9e9077454cec0.jpg)
SOLVED: Results: Calculate the heat gained by the water (lost by the substance in the calorimeter using the equation in the Introduction: Remember t0 write the unitsl! Q fon water using Ist
![PDF] Heat capacity and glass transition in P2O5-H2O solutions: support for Mishima's conjecture on solvent water at low temperature. | Semantic Scholar PDF] Heat capacity and glass transition in P2O5-H2O solutions: support for Mishima's conjecture on solvent water at low temperature. | Semantic Scholar](https://d3i71xaburhd42.cloudfront.net/e9e458615e33c40d94b80a3189efa26d438c8a39/3-Table1-1.png)
PDF] Heat capacity and glass transition in P2O5-H2O solutions: support for Mishima's conjecture on solvent water at low temperature. | Semantic Scholar
![Calculate the enthalpy change of freezing of 1.0 mol of water at 10^(@)C to ice at -10^(@)C, Delta(fus)H=6.03 kJ mol^(-1) at 0^(@)C. C(P)[H(2)O(l)]=75.3 J mol^(-1) K^(-1) C(P)[H(2)O(s)]=36.8 J mol^(-1) K^(-1) Calculate the enthalpy change of freezing of 1.0 mol of water at 10^(@)C to ice at -10^(@)C, Delta(fus)H=6.03 kJ mol^(-1) at 0^(@)C. C(P)[H(2)O(l)]=75.3 J mol^(-1) K^(-1) C(P)[H(2)O(s)]=36.8 J mol^(-1) K^(-1)](https://d10lpgp6xz60nq.cloudfront.net/web-thumb/34965050_web.png)
Calculate the enthalpy change of freezing of 1.0 mol of water at 10^(@)C to ice at -10^(@)C, Delta(fus)H=6.03 kJ mol^(-1) at 0^(@)C. C(P)[H(2)O(l)]=75.3 J mol^(-1) K^(-1) C(P)[H(2)O(s)]=36.8 J mol^(-1) K^(-1)
![The enthalpy change for a reaction at equilibrium is - 20.5 kJ mol ^-1 . Then the entropy change for this equilibrium at 410 K is: The enthalpy change for a reaction at equilibrium is - 20.5 kJ mol ^-1 . Then the entropy change for this equilibrium at 410 K is:](https://dwes9vv9u0550.cloudfront.net/images/4941372/74bbcad6-c829-4782-89bd-9e7db7c2f88e.jpg)